Question 1

Which of the following acids has the lowest pH? 0.1 M HBO, pKa = 2.43
0)1 M HA, pKa = 4.55
0)1 M HMO, pKa = 8.23
0)1 M HST, pKa = 11.89
Pure water

Accepted Answer

A)  HA 
B)  HST 
C)  HMO 
D)  HBO 
E)  pure water 
A)  HA 
B)  HST 
C)  HMO 
D)  HBO 
E)  pure water

Question 2

Which one of the following substances will give an aqueous solution of pH < 7?

Accepted Answer

A)  KI 
B)  NH4Br 
C)  Na2CO3 
D)  CH3COONa 
E)  CH3OH 
A)  KI 
B)  NH4Br 
C)  Na2CO3 
D)  CH3COONa 
E)  CH3OH

Question 3

Kw = 1.0 × 10-14, regardless of temperature.

Accepted Answer

A) True 
 B)False

Question 4

Define an acid according to the Arrhenius theory, and write a balanced equation to support this definition.

Accepted Answer

An acid is a substance which c

Question 5

The hydrated Al3+ ion, Al(H2O)63+, is a weak acid in water. What are the products of its reaction with H2O? Al(H2O)63+(aq) + H2O(l) F1F1F1S1F1F1F10 ?

Accepted Answer

A)  Al(H2O)5OH2+(aq) + H3O+(aq) 
B)  Al(H2O)6H4+(aq) + OH-( aq) 
C)  Al(H2O)53+(aq) + 2H2O(l) 
D)  Al(H2O)6OH2+(aq) + H3O+( aq) 
E)  Al(H2O)62+(aq) + H3O+( aq) 
A)  Al(H2O)5OH2+(aq) + H3O+(aq) 
B)  Al(H2O)6H4+(aq) + OH-( aq) 
C)  Al(H2O)53+(aq) + 2H2O(l) 
D)  Al(H2O)6OH2+(aq) + H3O+( aq) 
E)  Al(H2O)62+(aq) + H3O+( aq)

Question 6

The substance HCl is considered

Accepted Answer

A)  a weak Arrhenius acid. 
B)  a weak Arrhenius base. 
C)  a strong Arrhenius acid. 
D)  a strong Arrhenius base. 
E)  a neutral compound. 
A)  a weak Arrhenius acid. 
B)  a weak Arrhenius base. 
C)  a strong Arrhenius acid. 
D)  a strong Arrhenius base. 
E)  a neutral compound.

Question 7

If the compound HX is a strong acid (where H is the acidic proton in this acid), then the ion X- is a weak base.

Accepted Answer

A) True 
 B)False

Question 8

All Brønsted-Lowry bases have at least one lone pair of electrons.

Accepted Answer

A) True 
 B)False

Question 9

Which of the following aqueous liquids is the most acidic?

Accepted Answer

A)  0.1 M Al(NO3)3, Ka = 1 × 10-5 
B)  0.1 M Be(NO3)2, Ka = 4 × 10-6 
C)  0.1 M Pb(NO3)2, Ka = 3 × 10-8 
D)  0.1 M Ni(NO3)2, Ka = 1 × 10-10 
E)  pure water 
A)  0.1 M Al(NO3)3, Ka = 1 × 10-5 
B)  0.1 M Be(NO3)2, Ka = 4 × 10-6 
C)  0.1 M Pb(NO3)2, Ka = 3 × 10-8 
D)  0.1 M Ni(NO3)2, Ka = 1 × 10-10 
E)  pure water

Question 10

Ammonium chloride is used as an electrolyte in dry cells. Which of the following statements about a 0.10 M solution of NH4Cl, is correct?

Accepted Answer

A)  The solution is weakly basic. 
B)  The solution is strongly basic. 
C)  The solution is neutral. 
D)  The solution is acidic. 
E)  The values for Ka and Kb for the species in solution must be known before a prediction can be made. 
A)  The solution is weakly basic. 
B)  The solution is strongly basic. 
C)  The solution is neutral. 
D)  The solution is acidic. 
E)  The values for Ka and Kb for the species in solution must be known before a prediction can be made.

Question 11

Aqueous solutions of phosphoric acid and sodium nitrite are combined, and the following equilibrium is established. H3PO4(aq) + NO2-(aq)   H2PO4-(aq) + HNO2(aq)
The equilibrium constant Kc for this reaction is greater than one. Based on this information, which of the following statements is correct?

Accepted Answer

A)  Phosphoric acid is a weaker acid than nitrous acid. 
B)  Nitrous acid is a weaker acid than water. 
C)  The nitrite anion is a weaker base than the dihydrogen phosphate anion. 
D)  The dihydrogen phosphate anion is a stronger acid than nitrous acid. 
E)  Phosphoric acid is a stronger acid than nitrous acid. 
A)  Phosphoric acid is a weaker acid than nitrous acid. 
B)  Nitrous acid is a weaker acid than water. 
C)  The nitrite anion is a weaker base than the dihydrogen phosphate anion. 
D)  The dihydrogen phosphate anion is a stronger acid than nitrous acid. 
E)  Phosphoric acid is a stronger acid than nitrous acid.

Question 12

The English are fond of soggy French fries ("chips") wrapped in old newspaper and generously drenched in vinegar, which is a 0.83 M solution of acetic acid. If the acetic acid in vinegar is 0.47% dissociated, calculate Ka for this acid.

Accepted Answer

Question 13

What is the pH of a 0.0125 M NaOH solution?

Accepted Answer

A)  0.972 
B)  1.903 
C)  12.097 
D)  13.028 
E)  none of the above 
A)  0.972 
B)  1.903 
C)  12.097 
D)  13.028 
E)  none of the above

Question 14

Which of the following pairs has the stronger acid listed first?

Accepted Answer

A)  HBr, HI 
B)  HClO2, HClO3 
C)  H2SeO4, H2SeO3 
D)  HNO2, HNO3 
E)  HF, HCl 
A)  HBr, HI 
B)  HClO2, HClO3 
C)  H2SeO4, H2SeO3 
D)  HNO2, HNO3 
E)  HF, HCl

Question 15

Which of the following is considered a Lewis acid?

Accepted Answer

A)  CH3NH2 
B)  BCl3 
C)  F- 
D)  BF4- 
E)  CH4 
A)  CH3NH2 
B)  BCl3 
C)  F- 
D)  BF4- 
E)  CH4

Question 16

The ammonium ion, NH4+, is a weak acid.

Accepted Answer

A) True 
 B)False

Question 17

All Brønsted-Lowry bases contain the hydroxide ion, OH-.

Accepted Answer

A) True 
 B)False

Question 18

Which one of the following is a strong acid?

Accepted Answer

A)  H2CO3 
B)  H2SO3 
C)  H2SO4 
D)  H3PO4 
E)  CH3COOH 
A)  H2CO3 
B)  H2SO3 
C)  H2SO4 
D)  H3PO4 
E)  CH3COOH

Question 19

All weak acids have strong conjugate bases.

Accepted Answer

A) True 
 B)False

Question 20

An aqueous solution is prepared by dissolving the salt formed by the neutralization of a weak acid by a weak base. Which statement about the solution is correct?

Accepted Answer

A)  The solution is strongly basic. 
B)  The solution is weakly basic. 
C)  The solution is neutral. 
D)  The solution is acidic. 
E)  The values for Ka and Kb for the species in solution must be known before a prediction can be made. 
A)  The solution is strongly basic. 
B)  The solution is weakly basic. 
C)  The solution is neutral. 
D)  The solution is acidic. 
E)  The values for Ka and Kb for the species in solution must be known before a prediction can be made.

Exam 18: Acid-Base Equilibria

Which of the following acids has the lowest pH? 0.1 M HBO, pKa = 2.43 0)1 M HA, pKa = 4.55 0)1 M HMO, pKa = 8.23 0)1 M HST, pKa = 11.89 Pure water

Which one of the following substances will give an aqueous solution of pH < 7?

Kw = 1.0 × 10-14, regardless of temperature.

Define an acid according to the Arrhenius theory, and write a balanced equation to support this definition.

The hydrated Al3+ ion, Al(H2O)63+, is a weak acid in water. What are the products of its reaction with H2O? Al(H2O)63+(aq) + H2O(l)  ?

The substance HCl is considered

If the compound HX is a strong acid (where H is the acidic proton in this acid), then the ion X- is a weak base.

All Brønsted-Lowry bases have at least one lone pair of electrons.

Which of the following aqueous liquids is the most acidic?

Ammonium chloride is used as an electrolyte in dry cells. Which of the following statements about a 0.10 M solution of NH4Cl, is correct?

Aqueous solutions of phosphoric acid and sodium nitrite are combined, and the following equilibrium is established. H3PO4(aq) + NO2-(aq) H2PO4-(aq) + HNO2(aq) The equilibrium constant Kc for this reaction is greater than one. Based on this information, which of the following statements is correct?

The English are fond of soggy French fries ("chips") wrapped in old newspaper and generously drenched in vinegar, which is a 0.83 M solution of acetic acid. If the acetic acid in vinegar is 0.47% dissociated, calculate Ka for this acid.

What is the pH of a 0.0125 M NaOH solution?

Which of the following pairs has the stronger acid listed first?

Which of the following is considered a Lewis acid?

The ammonium ion, NH4+, is a weak acid.

All Brønsted-Lowry bases contain the hydroxide ion, OH-.

Which one of the following is a strong acid?

All weak acids have strong conjugate bases.

An aqueous solution is prepared by dissolving the salt formed by the neutralization of a weak acid by a weak base. Which statement about the solution is correct?

Keys to the Study of Chemistry

The Components of Matter

Stoichiometry of Formulas and Equations

The Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Thermochemistry: Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids, Solids, and Phase Changes

The Properties of Mixtures: Solutions and Colloids

Periodic Patterns in the Main Group Elements: Bonding, Structure, and Reactivity

Organic Compounds and the Atomic Properties of Carbon

Kinetics: Rates and Mechanisms of Chemical Reactions

Equilibrium: the Extent of Chemical Reactions

Ionic Equilibria in Aqueous Systems

Thermodynamics: Entropy, Free Energy, and the Direction of Chemical Reactions

Electrochemistry: Chemical Change and Electrical Work

The Elements in Nature and Industry

The Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

Which of the following acids has the lowest pH? 0.1 M HBO, pK_a = 2.43 0)1 M HA, pK_a = 4.55 0)1 M HMO, pK_a = 8.23 0)1 M HST, pK_a = 11.89 Pure water

K_w = 1.0 × 10^-14, regardless of temperature.

The hydrated Al³⁺ ion, Al(H₂O)₆³⁺, is a weak acid in water. What are the products of its reaction with H₂O? Al(H₂O)₆³⁺(aq) + H₂O(l)  ?

The substance HClis considered

If the compound HX is a strong acid (where H is the acidic proton in this acid), then the ion X^- is a weak base.

Ammonium chloride is used as an electrolyte in dry cells. Which of the following statements about a 0.10 M solution of NH₄Cl, is correct?

The English are fond of soggy French fries ("chips") wrapped in old newspaper and generously drenched in vinegar, which is a 0.83 M solution of acetic acid. If the acetic acid in vinegar is 0.47% dissociated, calculate K_a for this acid.

The ammonium ion, NH₄⁺, is a weak acid.

All Brønsted-Lowry bases contain the hydroxide ion, OH^-.